Associated with any ionic compound is the solubility product constant, which measures how soluble the compound will be in a solvent.

Concept #1: Understanding the Solubility Product Constant.

The general rule is that the greater the solubility product constant for a compound then the more soluble the compound.

Example #1: Consider the following compounds. Which has the highest concentration of OH^{-} ions?

a) Co(OH)_{2 }K_{sp} = 1.3 x 10^{-}^{15}

b) Cu(OH)_{2} K_{sp} = 2.2 x 10^{-20}

c) Ni(OH)_{2} K_{sp} = 6.0 x 10^{-16}

d) Fe(OH)_{2} K_{sp} = 4.1 x 10^{-15}

e) Zn(OH)_{2} K_{sp} = 3.0 x 10^{-16}

Example #2: The solubility of silver sulfate, Ag_{2}SO_{4}, is 0.025 M at 25^{o}C. Calculate its solubility product constant, K_{sp}.

Whenever the question refers to the solubility then that value represents our “x” variable.

Example #3: Find the solubility of CoCl_{3} (K_{sp} = 2.8 x 10^{-13}) in:

a) pure water

Whenever we deal with the solubility product constant we use an ICE Chart and since the reactant will always be a solid then we can ignore it.

If our compound dissolves in a solution with similar ions then the **Common Ion Effect** takes place.

Example #4: Find the solubility of CoCl_{3} (Ksp = 2.8 x 10^{-13}) in:

b) 0.20 M NaCl.

Example #5: What is the molar solubility of Fe(OH)_{3} (s) in a solution that is buffered at pH 3.50 at 25 ^{o}C? The *K*sp of Fe(OH)_{3} is 6.3 x 10** ^{–38}** at 25

Example #6: Find the pH of a saturated solution of Aluminum hydroxide, Al(OH)_{3}. The K_{sp} of Al(OH)_{3} is 1.9 x 10** ^{-10}**.

Example #7: Will a precipitate form when 0.150 L of 0.100 M Pb(C_{2}H_{3}O_{2})_{2} and 0.100 L of 0.20 M KCl are mixed? The K_{sp} value of PbCl_{2} is 1.2 x 10** ^{-5}**.

Example #8: Two flasks containing 7.12 x 10** ^{-6}** M silver nitrate, AgNO

- A precipitate of Sr(NO
_{3})_{2}will form. - The solution is saturated but will remain clear.
- The solution is not saturated and no precipitate will form.
- A precipitate of silver bromide will form, with silver and bromide ions as well.
- A precipitate of silver bromide will form.

Example #9: A saturated solution of AlCl_{3} contains 5.15 x 10** ^{-4}** M chloride ions. What is the solubility product constant, K

Example #10: Molar Solubility of Ions

Example #11: The solubility of CaF_{2} is 53.2 g/mL at 25 ** ^{o}**C. Calculate its solubility product constant, Ksp.

Example #12: The concentration of chloride and iodide ions present in the solution are [Cl^{ –}] = 0.073 M and [I^{ –}] = 0.060 M. The use of silver, Ag, can be used to precipitate these two ions. If the K_{sp} value of AgCl is 1.77 x 10** ^{-10}** and AgI is 8.51 x 10

a) Which ion will precipitate out first?

b) At what concentration will this ion from Part A begin to precipitate out?

Which reagent can be used to separate silver and copper from an aqueous solution of AgNO3 and Cu(NO3)2?
a. 1.0 M H2SO4
b. 1.0 M HCl
c. 1.0 M NaCl
d. b and c
e. all of the above

Which reagent can be used to separate cobalt and copper from an aqueous solution of Co(NO3)2 and Cu(NO3)2?
a. 5% thioacetamide in HNO3 (aq), heated to ~80°C
b. 1.0 M HCl
c. 1.0 M NH3
d. a and b
e. a and c

Which reagent can be used to separate the solids Al(OH) 3 and Fe(OH)3?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NaCl
d. a and b
e. none of the above

Arrange the compounds in increasing order of molar solubility.

The Ksp equation for sodium bicarbonate (NaHCO3) should be written as:

Determine the molar solubility of Al(OH)3 in a solution containing 0.050 M KOH.
Ksp (Al(OH)3) = 1.9 x 10 -33
A) 1.0 x 10-11 M
B) 5.0 x 10-7 M
C) 4.75 x 10-36 M
D) 1.5 x 10-29 M
E) 0.050 M

Give the expression for the solubility product constant for Hg 2Cl2.
A) [Hg22+][Cl-]2 / [Hg2Cl2]
B) [Hg2Cl2] / [Hg22+][Cl-]2
C) [Hg22+][Cl1-]2
D) [Hg22+]2[Cl-] / [Hg2Cl2]
E) [Hg22+]2[Cl1-]

What is the minimum S2− concentration that will cause ZnS to start precipitating from a 0.10 M solution of Zn(NO3)2, a very soluble salt? Ksp for ZnS is 1.1 × 10−21.

Determine the molar solubility of some salt with the generic formula AB 2 if Ksp = 2.56x102 .
10 M
0.1 M
4 M
1 M

A hypothetical compound MX3 has a molar solubility of 0.00562 M. What is the value of Ksp for MX3?
3.16 x 10-5
2.99 x 10-9
9.48 x 10-5
2.69 x 10-8

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K sp (AgBr) = 7.7 × 10-13.

The solubility of CaCO3 (formula weight 100.1) is 0.0095 g in 1800 mL. What is the Ksp?
A. 2.8 x 10 -5
B. 2.8 x 10 -9
C. 5.2 x 10 -5
D. 5.2 x 10 -9
E. 3.8 x 10 -7

The concentration of silver ions, [Ag+], in a saturated solution of Ag 2CO3 is 2.5x10-4 M at 25.0°C. Determine the Ksp for Ag 2CO3 at this temperature.
A. 5.0 x 10-10
B. 1.3 x 10-7
C. 3.1 x 10-8
D. 6.3 x 10-11
E. 7.8 x 10-12

What is the pH of a standard solution of iron (II) hydroxide, Fe(OH) 2. Ksp = 4.87 x 10-17 for the Iron (II) hydroxide.
a. 5.64
b. 8.36
c. 5.34
d. 8.66
e. 8.76

How many grams of CuCl (MW = 99.0 g mol –1) can be dissolved in 5.00 L of water before a precipitate forms? Ksp(CuCl) = 1.0 x 10–6
(a) 0.10 g
(b) 0.22 g
(c) 0.49 g
(d) 0.98 g
(e) 1.10 g

Describe the solubility of Al(OH)3 with respect to pH.
A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
B) soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH
C) insoluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
D) insoluble at low pH, in pH-neutral solution, and at high pH
E) pH has no effect on the solubility

The solubility of silver (I) iodate is 0.0027 g/100 mL at 20 oC. What is the solubility product for silver iodate? (MWt AgIO3 = 273 g/mole)
A) 1.0 × 10–8
B) 3.9 × 10–6
C) 9.8 × 10–9
D) 2.7 × 10–12
E) 1.4 × 10–3

What is the molar solubility of barium nitrate, Ba(NO 3)2, which has a Ksp value of 4.6 × 10−3 ?

Which is the ion product expression for magnesium ammonium phosphate, MgNH4PO4.
a) [Mg2+][NH4+][PO43-]
b) [PO43-] / [Mg2+][NH4+]
c) [Mg2+NH4+][PO43-]
d) [Mg2+][NH4+] / [PO43-]
e) 1 / [Mg2+][NH4+][PO43-]

Solve for the concentration of Magnesium ions when 1.29 moles of Mg(OH) 2) is added to a 1.00 L solution that is initially at pH = 11.00. Ksp (Mg(OH)2) = 5.6 X 10-12
A. 5.6 X 10-9
B. 5.6 X 10-6
C. 1.1 X 10-5
D. 1.1 X 10-4
E. 1.3

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.
Ksp (CuCl) = 1.0 x 10-6
A) 1.0 x 10-12 M
B) 5.0 x 10-7 M
C) 2.0 x 10-5 M
D) 1.0 x 10-3 M
E) 0.050 M

Which of the following compounds will have the highest molar solubility in pure water?
A) PbSO4, Ksp = 1.82 x 10-8
B) MgCO3, Ksp = 6.82 x 10-6
C) AgI, K sp = 8.51 x 10-17
D) PbS, K sp = 9.04 x 10-29
E) FeS, K sp = 3.72 x 10-19

What is the ksp expression for Mg 3(PO4)2? (Look at all the answers carefully. Some of them are very similar)
(a) [Mg2+]3[PO43-]2
(b) [Mg2+]2[PO43-]3
(c) [Mg]3[PO4]2
(d) [Mg]3[PO4]2
[Mg3(PO4)2]
(e) [Mg3(PO4)2]
[Mg]3[PO4]2

Would you expect the solubility of Mg 3(PO4)2 to be greater than, less than, or the same in a 0.10 M Na3PO4 solution compared to pure water?
(a) greater than (b) less than (c) the same

Which of the following solubility product expressions is incorrect?
A. Ksp (Ag2S) = [Ag+]2[S-2]
B. Ksp ( CaF2) = [Ca2+][F-]2
C. Ksp (PbCl2) = [Pb2+][Cl-]2
D. Ksp (CuS) = [Cu2+][S2-]
E. Ksp (Ag3PO4) = [Ag+]3[P] [O3-]4

What is the solubility product, Ksp of Mg(OH)2 if its solubility in water is 1.6 x 10 -4 mol•L-1?
a) 1.6 x 10-11
b) 2.6 x 10-8
c) 3.2 x 10-4
d) 4.1 x 10-12

A saturated solution of MgF2 contains 1.6 x 10-3 mol of MgF2 per liter at a certain temperature. What is the Ksp, of MgF2 at this temperature?
a) 2.7 x 10-6
b) 1.6 x 10-8
c) 3.1 x 10-9
d) 6.2 x 10-9

The addition of solid Na 2SO4 to an aqueous solution in equilibrium with solid BaSO 4 will cause
a) no change in [Ba 2+] in solution.
b) more BaSO4 to dissolve.
c) precipitation of more BaSO4.
d) an increase in the Ksp of BaSO4.

The solubility of lead (II) iodide is 0.064 g / 100 mL at 20°C. What is the solubility product for lead (II) iodide?
A) 1.1 x 10-8
B) 3.9 x 10-6
C) 1.1 x 10-11
D) 2.7 x 10-12
E) 1.4 x 10-3

Calculate the molar solubility of silver (I) carbonate ( Ksp=8.1x10–12) in water at 25 ̊C.
a. 8.1x10–12 M
b. 2.0x10–6 M
c. 1.3x10–4 M
d. 1.6x10–4 M
e. 2.6x10–4 M

Calcium hydroxide has a molar solubility of 0.0118 M in water. How much Ca(OH) 2 (in mg) is soluble in 100.0 mL of water?
a. 6.5x10–6 mg
b. 0.0118 mg
c. 0.0235 mg
d. 0.874 mg
e. 87.4 mg

Calculate the solubility of silver oxalate, Ag 2C2O4, in pure water. [Ksp = 1.0 x 10-11]
A) 1.4 x 10-4 M
B) 8.2 x 10-5 M
C) 5.4 x 10-5 M
D) 3.2 x 10-6 M
E) 2.5 x 10-12 M

The Ksp of PbBr2 is 6.60 x 10-6
i) What is the molar solubility(M) of PbBr2 in pure water?
ii) What is the molar solubility(M) of PbBr2 in 0.500M KBr solution?
iii) What is the molar solubility(M) of PbBr2 in a 0.500M Pb(NO3)2 solution?

Write and compare the Ksp expressions for ionic compounds of composition AB 2 and C2D3.

What is the molar solubility of a saturated solution of PbCl 2 (Ksp=1.7x10–5)?
a. 1.5x10–5 M
b. 2.9x10–3 M
c. 4.1x10–3 M
d. 0.016 M
e. 0.020 M

6.5 mg of calcium fluoride is soluble in 250.0 mL of water at 25 ̊C. What is its Ksp?
a. 1.1x10–7
b. 1.5x10–10
c. 3.7x10–11
d. 2.3x10–12
e. 5.8x10–13

What pH should an aqueous solution of Co(OH) 2 (Ksp=1.1x10–15) be adjusted to so that the concentration of Co2+ is 1.0 x 10–9 M.
a. 8.04
b. 8.81
c. 10.72
d. 11.02
e. 11.32

Two compounds with general formulas AX and AX 2 have Ksp = 1.5 x 10 -5. Which of the two compounds has the higher molar solubility? Explain your choice.

What is the pH of a saturated aqueous solution of Cd(OH) 2 (Ksp=2.5x10–14)?
a. 9.57
b. 9.47
c. 9.27
d. 7.35
e. 4.73

What is the molar solubility of silver (I) carbonate ( Ksp=8.1x10–12) in the presence of 0.20 M Na2CO3?
a. 3.18 × 10−6 M
b. 4.50 × 10−6 M
c. 1.27 × 10−4 M
d. 1.42 × 10−5 M
e. 5.68 × 10−5 M

A solution begins with 0.100 M of NaF dissolved in water. What is the concentration of Magnesium ion in the solution, if MgF2 was added in excess? Ksp (MgF2) = 5.2 X 10 −11
A. 5.2 * 10−13
B. 5.2 * 10 −11
C. 5.2 * 10 −9
D. 0.00023
E. 0.00047

In which of the following solutions would PbBr2 be expected to be the least soluble at a given temperature.
A. 0.1M CaBr2
B. 0.1M HBr
C. 0.1M NaBr
D. 0.1M KNO3

Which of the following compounds will have the highest molar solubility in pure water?
A. NiS Ksp = 3.00x10 -20
B. PbS Ksp = 9.04x10 -29
C. MgCO3 Ksp = 6.82x10 -6
D. AgCN Ksp = 5.97x10 -17
E. PbSO4 Ksp = 1.82x10 -8

In which solution is Ag3PO4 least soluble?
a. In pure water
b. 0.50 M AgNO3
c. 0.50 M Na3PO4
d. AgPO4 is least soluble equally in b and c
e. AgPO4 is equally soluble in all of the above

Give the expression for the solubility product constant for BaF 2.

Given the following Ksp values, which statement about solubility in water is correct?
K sp
PbCrO4 2.0 x 10 -16
Zn(OH)2 4.5 x 10 -17
Pb(OH)2 1.2 x 10 -15
MnS 2.3 x 10 -13
a) PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubility in water.
b) PbCrO4 has the lowest solubility in water.
c) The solubility of MnS in water will not be pH dependent.
d) MnS has the highest molar solubility in water.
e) A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution.

What is the molar solubility of silver (I) carbonate in the presence of 0.20 M Na 2CO3?
a. 3.18 x 10 -6M
b. 4.50 x 10 -6M
c. 1.27 x 10 -4M
d. 1.42 x 10 -5M
e. 5.68 x 10 -5M

Which of the following salts has the highest concentration of silver ion when dissolved in water?
a) AgCl Ksp = 1.6 x 10-10
b) Ag2CO3 Ksp = 8.1 x 10-12
c) AgBr Ksp = 5.0 x 10-13

Which of the following compounds has the lowest solubility in water?
A. AgI, Ksp = 8.5 × 10 −17
B. PbBr2, Ksp = 6.6 × 10 −6
C. Sr3(PO4)2, Ksp = 4 × 10 −28
D. Ag(CH3COO), Ksp = 4.4 × 10 −3

Ksp = 4.64 × 10 −3 for Ba(NO3)2. What is the concentration of the nitrate ion in a saturated Ba(NO3)2 solution?
A. 0.105 M
B. 0.167 M
C. 0.210 M
D. 0.333 M
E. 0.068 M
F. 0.136 M

Which salt precipitates first and what is the minimum concentration of Ag + necessary to cause this precipitation in a solution containing 7.5 mL of 0.025 M NaCl and 7.5 mL of 0.025 M Na3PO4?
(Hint: dilution occurs)
Ksp(AgCl) = 1.8 x 10-10
Ksp(Na3PO4) = 1.3 x 10-20
a) AgCl 8.7 x 10 -7 M
b) Ag3PO4 2.3 x 10 -7 M
c) AgCl 1.4 x 10 -8 M
d) Ag3PO4 7.2 x 10 -8 M
e) None of these answers are correct

When a solution of weak electrolyte is altered by adding one of its ions from another source, the ionization of the weak electrolyte is suppressed. The behavior is termed the ___________.

In which of the following solutions would PbBr 2 be expected to be the least soluble at a given temperature?
0.1M CaBr2
0.1M HBr
0.1M NaBr
0.1M KNO3

AgCl would be least soluble at 25°C in ______ .

A solution of sodium fluoride is added dropwise to a solution that is 0.0144 M in ionic barium. At what concentration of fluoride ion will barium fluoride start to precipitate? Neglect volume changes, the Ksp for barium fluoride is 1.7x10 –6.
A. 2.4 x 10 –8
B. 1.1 x 10 –2
C. 1.2 x 10 –4
D. 5.9 x 10 –5
E. 2.7 x 10 –3

The solubility of PbBr2 is 8.44 g/L at 20◦C. What is Ksp for this compound?
A. 1.1 × 10 −6
B. 5.3 × 10 −4
C. 1.0 × 10 −3
D. 4.9 × 10 −5
E. 1.2 × 10 −5

Which reagent(s) INCREASES the solubility of Zn(OH) 2 when added to a saturated aqueous solution of Zn(OH)2?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NH 3
d. a and c
e. all of the above

You have an aqueous solution that contains a wide array of different ions along with a solid chunk of Ag3PO4 (Ksp = 9.8 × 10 −21) in it. The concentration of PO 43− in the solution is 2.0 × 10 −2 M. What is the concentration of the silver ion?
A. 9.9 × 10 −6 M
B. 4.4 × 10 −6 M
C. 7.9 × 10 −7 M
D. 2.6 × 10 −7 M
E. 2.3 × 10 −6 M

Which reagent(s) DECREASES the solubility of Ni(OH) 2 when added to a saturated aqueous solution of Ni(OH)2?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NiCl 2
d. a and c
e. all of the above

Which of the following compounds will have the highest molar solubility in pure water?
NiS Ksp = 3.00x10 –20
PbS Ksp = 9.04x10 –29
MgCO3 Ksp = 6.82x10 –6
AgCN Ksp = 5.97x10 –17
PbSO4 Ksp = 1.82x10 –8

What is the molar solubility of magnesium hydroxide in a basic solution with pH of 12.50? The Ksp for magnesium hydroxide is 5.6 x 10-12.
2.40x10-6 M
1.10x10-4 M
1.80x10-10 M
5.60x10-9 M

Solutions of 0.00024 M aqueous sodium iodide and 0.0054 M aqueous lead (II) nitrate, Pb(NO3)2 are mixed together. Which of the following is the most likely result that a student would observe? Assume no volume change. Ksp of Pbl2 is 1.4 x 10-8.
A. All ions remain in solution and no precipitate is observed.
B. A precipitate of sodium nitrate, NaNO3, is observed.
C. A precipitate of lead (II) iodide, Pbl 2, is observed.
D. The mixture results in the formation of a saturated solution at equilibrium.
E. The Nal and Pb(NO3)2 solutions do not mix and two separate layers are formed.

Enter the Ksp expression for the solid AB 2 in terms of the molar solubility x. Express your answer in terms of x.

If 147 g of ZnF2 (Ksp = 0.0300) is added to water to make a 1.00 L solution, what is the [F− ] concentration in the solution in molarity?
A. 0.173
B. 0.196
C. 0.391
D. 1.42
E. 2.84

A solution begins with 0.100 M of NaF dissolved in water. What is the concentration of Magnesium ion in the solution, if MgF2 was added in excess? Ksp (MgF2) = 5.2 X 10 −11
A. 5.2 x 10 −13
B. 5.2 x 10 −11
C. 5.2 x 10 −9
D. 0.00023
E. 0.00047

The molar solubility of Cd(OH)2 in water is 1.7 x 10 -5 mol/L at 25°C. The Ksp value for Cd(OH)2 is:
A. 2.0 x 10 -14
B. 4.9 x 10 -15
C. 5.8 x 10 -10
D. 2.9 x 10 -10
E. none of these

Silver iodide has very low solubility as shown by the following reaction equation.
Agl (s) ↔ Ag+ (aq) + I - (aq)
Which of the following statements is/are true?
i. K < l
ii. the concentration of Ag+ will be large
iii. K > l
a. i only
b. ii only
c. iii only
d. i and ii
e. ii and iii

Which of the following salts shows the lowest solubility in water?
Ksp values are as follows:
Ag2S = 1.6 x 10 -49
Bi2S3 = 1.0 x 10 -72
HgS = 1.6 x 10 -54
Mg(OH)2 = 8.9 x 10 -12
MnS = 2.3 x 10 -13
A. Bi2S3
B. Ag2S
C. MnS
D. HgS
E. Mg(OH)2

The solubility of CaF2 (s) [Ksp= 4.0 x 10 -11] in 1.0 L of a 1.0 x 10 -2 M solution of NaF is:
A. 4.0 x 10 -9 moles
B. 1.0 x 10 -7 moles
C. 7.0 x 10 -4 moles
D. 4.0 x 10 -7 moles
E. none of these

The concentration of OH - in a saturated solution of a certain metal hydroxide, M(OH)2 , is 3.6x10 -4 M . The Ksp of M(OH)2 is:
A. 1.3 x 10 -7
B. 4.7 x 10 -11
C. 1.2 x 10 -11
D. 3.6 x 10 -4
E. none of these

What is the molar solubility of Co(OH) 2 when buffered at a pH of 13.20?
a. 1.4 x 10 -5 M
b. 8.5 x 10 -6 M
c. 1.6 x 10 -12 M
d. 1.0 x 10 -13 M
e. 1.6 x 10 -14 M

Which salt is NOT more soluble in acidic solution than it is in pure water?
a. CdCO3 Ksp = 5.2 x 10 -12
b. Cd(OH)2 Ksp = 2.5 x 10 -14
c. Cd(OH)2 Ksp = 2.5 x 10 -15
d. AgI K sp = 8.3 x1 0 -17
e. ZnCO3 Ksp = 1.4 x 10 -11

C2D3 has a solubility product constant of 9.14 x 10 -9. What is the molar solubility of C2D3?

What is the pH in a saturated solution of hypothetical metal (III) hydroxide, M(OH) 3, Ksp = 1.9 x 10-16?
A. 3.81
B. 10.19
C. 9.71
D. 4.29
E. 10.31

Express Ksp in terms of molar solubility, x, for a salt with a formula of
i) AB(s)
ii) AB2(s)
iii) AB3(s)
iv) A3B2(s)

If the Ksp of a Ag3PO4 is 1.8 x 10-18, what is the silver ion concentration in a saturated solution of silver phosphate?a. 4.8 x 10 -5 Mb. 1.2 x 10 -5 Mc. 1.6 x 10 -5 Md. 3.2 x 10 -5 M

The Ksp for Ag3PO4 is 1.8 x 10-18. Calculate the molar solubility of Ag 3PO4.

Consider the following chemical equation:AaBb(s) → aA+(aq) + bB-(aq)In this case, the Ksp is given by:a. Ksp = a [A+] b [B-]b. Ksp = ([A+] / a) ([B-] / b)c. Ksp = [A+] [B-] / [AaBb]d. Ksp = [A+]a [B-]be. Ksp = [A+]a [B-]b / [AaBb]

The equilibrium constant for the reaction:Ag2SO4(s) ⇌ 2Ag+ (aq) + SO42- (aq)is Kc = 1.8x10 −10. If the SO42- concentration is 1.2x10−6 M, what is the Ag+ concentration?a) 0.221b) 1.50x10 −4c) 2.25x10 −8d) 1.22x10 −2e) 8.66x10 −6

What concentration of SO32- is in equilibrium with Ag 2SO3(s) and 2.90 x 10-3 M Ag+? The Ksp of Ag2SO3 can be found here: 1.5 x 10-14.

Calculate the molar solubility of barium fluoride in each of the following. Express all answers using three significant figures.Part A pure water.Part B 0.10 M Ba(NO3)2Part C 0.15 M NaF

Consider the reactionYZ(s) ⇌ Y(aq) + Z(aq)at equilibrium. If Ksp < [Y][Z], precipitation occurs.The reaction quotient, Q, is also equal to [Y][Z]. Q is equal to Ksp only at equilibrium. When Q is less than Ksp, the solution is unsaturated; when Q is greater than Ksp the solution is supersaturated and precipitation could occur.a. Enter the Ksp expression for A 2B3(s) in terms of [A] and [B].b. Enter the Ksp expression for AC 4(s) in terms of [A] and [C].Express your answer in terms of [A] and [C].

Enter the Ksp expression for A2B3(s) in terms of [A] and [B].

Enter the Ksp expression for AC4(s) in terms of [A] and [C].

Enter the solubility-product expression for Al(OH)3(s).

What is the correct expression for the solubility product constant for iron (III) hydroxide?
(a) Ksp = [Fe3+(aq)] [OH− (aq)]
(b) Ksp = [Fe3+(aq)] [OH− (aq)] 3
(c) Ksp = [Fe3+(aq)] 3 [OH− (aq)]
(d) Ksp = [Fe3+(aq)] 3[OH− (aq)]
(e) Ksp = [Fe3+(aq)] 3 [OH− (aq)] 3

The Ksp for PbI2(s) is 1.4 x 10-8. Calculate the solubility of PbI 2(s) in 0.075 M Nal.

Calculate the molar solubility of lead thiocyanate in 0.500 M KSCN?

Silver Chromate (Ag2CrO4, 331.73 g/mol) has a Ksp of 1.12 x 10 -12.
a) Calculate the solubility (in g/L) of silver chromate in water.
b) Calculate the solubility (in g/L) of silver chromate in 0.110 M AgNO 3 solution.

a) Write a balanced equation for the dissolution of CaCO 3.
b) Write an expression for Ksp for the dissolution of CaCO3.

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, 14.0? The Ksp is 4 x 10-16.

i) What is the solubility of M(OH) 2 in pure water? Ksp = 5.45 x 10 -18
ii) What is the solubility of M(OH) 2 in a .202 M solution of M(NO 3)2?

What is Ksp for PbCrO4, if its molar solubility is 1.3 × 10−7 mol/L?

Solid silver phosphate is allowed to equilibrate with water at 25°C until the solution is saturated. What is the silver ion concentration in this saturated solution? Ksp for Ag3PO4 is equal to 8.9 × 10−17 .

Enter the Ksp expression for C2D3 in terms of the molar solubility x.

Give the expression for the solubility product constant for PbCl 2.a. [Pb2+][Cl-]2b. [Pb2+]2[Cl-] / [PbCl2]c. [PbCl2] / [Pb2+][Cl-]2d. [Pb2+]2[Cl-]e. [Pb2+][Cl-]2 / [PbCl2]

What is the value of Q when the solution contains 2.50x103 M Mg2+ and 2.00x103 M CO32?

Calculate the molar solubility of CaF2. Given; Ksp = 4.0 x 10 -11.

What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbF2 from a solution that is 1.00x102 M in the fluoride ion, F? Ksp for lead(II) fluoride is 3.3x108.

Silver carbonate, Ag2CO3 is a salt of low solubility. When placed in water, it dissolves until an equilibrium is reached:
Ag2CO3 (s) ⇋ 2 Ag+ (aq) + CO32- (aq).
Write an expression for the solubility product constant, Ksp, of Silver Carbonate?

The Ksp value for silver carbonate, Ag 2CO3 , is 8.10 x 10 -12. Calculate the solubility of Ag2CO3 in grams per liter.

What concentration of SO32– is in equilibrium with Ag2SO3(s) and 1.00 × 10-3 M Ag+?

Write a balanced equation for the dissolution of PbCl 2.
Express your answer as a chemical equation. Identify all of the phases in your answer.

The Ksp of zinc hydroxide, Zn(OH)2, is 3.00 x 10 -17. Calculate the molar solubility of this compound.

Select the false statement below regarding PbI 2 (Ksp = 7.9 x 109) and PbCO3 (Ksp = 7.4 x 1014).A. the molar solubility of PbI 2 can be calculated by taking the cube root of (K sp/4)B. PbCO3 is more soluble in 1.0 M HCl than in pure waterC. PbI2 is less soluble in 1.0 M NaI than in pure waterD. PbCO3 is more soluble in 1.0 M Pb(NO 3)2 than in pure waterE. PbI2 is more soluble in 1.0 M NaOH than in pure water (Kf of Pb(OH) 2 = 8 x 1013)

Barium hydroxide, Ba(OH)2, is reported to have a Ksp of 2.55 x 10-4 at 25 degrees celsius.
a. What is the molar solubility of Ba(OH) 2?
b. What is the solubility of Ba(OH) 2 in g/L?

Calculate the molar solubility of CuX (K sp = 1.27 x 10 -36) in each of the following.
a. - 0.26 M CuCl 2
b. - 0.19 M Na 2X

Silver Chromate, Ag2CrO4, has a Ksp of 9.0 x 10 -12. Calculate the solubility, in moles per liter, of silver chromate.

Write a balanced equation for the dissolution of AgI.
Express your answer as a chemical equation. Identify all of the phases in your answer.

Calculate the molar solubility of Ni(OH) 2 when buffered at pH = 8.0. Express your answer using one significant figure.

If 147 g of ZnF2 (K sp = 0.0300) is added to water to make a 1.00 L solution, what is the [F− ] concentration in the solution in molarity?
A. 0.173
B. 0.196
C. 0.391
D. 1.42
E. 2.84

Silver sulfate (Ag2SO4) is an ionic solid that is only slightly soluble in water. When it is added to water, the reaction Ag2SO4(s) ⇌ 2 Ag+(aq) + SO42–(aq) takes place.
A large amount of Ag2SO4(s) is placed in water at 25°C. Some of it dissolves and the solution at equilibrium contains 0.029 M Ag+(aq). What is the equilibrium constant for the reaction
Ag2SO4(s) ⇌ 2 Ag+(aq) + SO42–(aq)?
A) 1.8 x 10–7
B) 6.1 x 10–6
C) 1.2 x 10–5
D) 2.4 x 10–5
E) 8.4 x 10–4

The Ksp of iron(II) hydroxide, Fe(OH)2, is 4.87 x 10-17. Calculate the solubility of this compound in g/L.

Complete the following reaction table and Ksp expression to calculate the solubility of silver chloride.

The solubility of silver sulfate (MW 311.8) is 4.73 g/L at 25°C. Calculate solubility product constant.
a) 1.4 x 10-5
b) 6.5 x 10-8
c) 2.3 x 10-4
d) 8.1 x 10-9
e) 3.4 x 10-6

Enter the solubility-product expression for Mg 3(PO4)2(s). Include Charges.

The solubility of lead(II) bromide, PbBr2, in water is 4.34 g/L. In an aqueous solution an equilibrium exists between the dissolved ions and the solid salt.
PbBr2(s) ⇋ Pb2+(aq) + 2 Br -1 (aq)
a) write the solubility product expression for this equation.
b) calculate the molar concentration and the Ksp ( solubility product constant) for lead(II) bromide.

The Ksp of AgCl is 1.6 x 10-10. What is the solubility of AgCl in 0.10 M AgNO 3?

A saturated solution of lead(II) iodide, PbI 2 has an iodide concentration of 3.0 x 10 -3 mol/L.
a) What is the molar solubility of PbI2?
b) Determine the solubility constant, Ksp, for lead (II) iodide.
c) Does the molar solubility of lead (II) iodide increase, decrease, or remain unchanged with the addition of potassium iodide to the solution? Explain.

Solid aluminum phosphate, AlPO4, is in equilibrium with its ions in solution:
AlPO4 ↔ Al +3 +PO4 3- with Ksp = 1 x10 -22
HINT: Note the definition of "solubility product".
Find the concentration of phosphate ions (in mg/L)

What is the value of Q when the CaSO4 solution contains 2.00×10−3M Ca+2 and 3.00×10-2M SO42-?Express your answer numerically.

a. Use the molar solubility 1.08 × 10 −5 M in pure water to calculate Ksp for BaCrO4.
b. Use the molar solubility 1.55 × 10 −5 M in pure water to calculate Ksp for Ag2SO3.
c. Use the molar solubility 2.22 × 10 −8 M in pure water to calculate Ksp for Pd(SCN)2.

0.150 M Na 2SO4 solution that is saturated with Ag 2SO4 has [Ag+] = 9.7 times 10 -3 M.
What is the value of Ksp for Ag2SO4 obtained with these data? Express your answer using two significant figures.

The solubility product, Ksp, for PbCl2 is 1.7 × 10–5. What is the solubility of PbCl 2 in water, in moles per litre?
a. 1.6 × 10–2 mol L–1
b. 6.2 × 10–2 mol L–1
c. 2.4 × 10–4 mol L–1
d. 7.7 × 10–3 mol L–1

Enter the Ksp expression for the solid AB2 in terms of the molar solubility x. express your answer in terms of x.

The Ksp of AgCl is 1.6 x 10 -10. What is the solubility of AgCl in 0.0010 M FeCl 3?

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. BaSO4b. PbBr2c. Ag2CrO4

a. Use the molar solubility 1.08 x 10 -5 in pure water to calculate Ksp for BaCrO4.
b. Use the molar solubility 1.55 x 10 -5 in pure water to calculate Ksp for Ag2SO3.
c. Use the molar solubility 2.22 x 10 -8 in pure water to calculate Ksp for Pd(SCN)2.

What is the Ksp of Al(OH)3 if the concentration of OH- in a saturated solution of Al(OH)3 is 1.6 x 10-8 M? a. 2.6 x 10-16 b. 1.6 x 10-23c. 1.8 x 10-30 d. 2.2 x 10-32

What concentration of SO32- is in equilibrium with Ag2SO3(s) and 9,80 x 103 M Ag+ The Ksp of Ag2SO3 can be found here.

If the concentration of Mg2+ ion in seawater is 1270 mg/L, what OH- concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) = 5.6 times 10-12

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca^2+ (aq) and 0.0320 M Ag^+(aq). What will be the concentration of Ca^2+(aq) when Ag2SO4(s) begins to precipitate? What percentage of the Ca^2+(aq) can be precipitated from the Ag^+(aq) by selective precipitation?

A generic salt, AB, has a molar mass of 197 g/mol and a solubility of 1.40 g/L at 25 °C. What is the Ksp of this salt at 25 °C?AB(s) <-->A +(aq) + B- (aq)

Copper(I) ions in aqueous solution react with NH3(aq) according toCu+(aq) + 2 NH3(aq) → Cu(NH3)2+(aq) Kf = 6.3x1010 Calculate the solubility (in g• L-1) of CuBr(s) (Ksp = 6.3x10-9) in 0.73 M NH3(aq).

At 25°C only 0.0300 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB3(s) ⇌ A3+(aq) + 3 B-(aq)

Estimate the solubility of lead(II) bromide in a. moles per liter of pure water. b. in grams per liter of pure water.Ksp for lead(II) bromide is 6.6 times 10-6.

What concentration of SO32- is in equilibrium with Ag2SO3 (s) and 3.10 x 10-3 M Ag+? The Ksp of Ag2SO3 can be found here.

Write the solubility product expression for the following compound Ni(OH) 2Ksp = ____

At 25 °C only 0.0790 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?AB (s) ⇌ A+ (aq) + B- (aq)

What is the molar solubility of calcium carbonate (CaCO3) in water? The solubility-product constant for CaCO3 is 4.5 x 10^-9 a. 9.0 x 10^-9 b. 9.5 x 10^-5 c. 8.35 d. 2.3 x 10^-9 e. 6.7 x 10^-5

Based on the given value of the K_sp what is the molar solubility of Mg(OH)2 in 0.190 M NaOH?

The Ksp of cobalt (ll) hydroxide, Co(OH)2, is 5.92 x10 ^-15. Calculate the molar solubility of this compound.

Determine the relative solubilities of the following compounds:

The Ksp of CaSO4 is 4.93 times 10-5. Calculate the solubility (in g/L)of CaSO4(s) in 0.300 M Na2SO4(Aq) at 25 °C.

A solution of saturated PbF2 is found to contain 4.0 x 10-3 M fluoride ion. Calculate the Ksp of PbF2.

For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g., ABC.) Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water.

The solubility product constant for MX 2 is 2.5 x 10-8. How many grams of MX 2 (104.67 g/mol) will dissolve in 136 ml of water at 25°C. M is the metal and X is the anion.

At 25°C only 0.0100 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB (s) ⇌ A+ (aq) + B- (aq)

A generic salt, AB2, has a molar mass of 341 g/mol and a solubility of 4.60 g/l at 25 °C. What is the Ksp this salt at 25 °C? AB2(s) ⇌ A2+(aq) + 2B -(aq)

At 25°C only 0.0720 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB2 (s) ⇌ A2+ (aq) + 2B- (aq)

he Ksp of cerium (ll) iodate, Ce(lO3)3 is 1.40 x 10-11. Calculate the molar solubility of this compound.

The solubility of Ag2S is measured and found to be 7.10 x 10-15 g/L. Use this information to calculate a Ksp value for silver sulfide.

Which of the following substances has the greatest solubility in water? a. MgCO3, Ksp = 3.5 x 10-8b. NiCO3, Ksp = 1.3 x 10-7 c. AgIO3, Ksp = 3.1 x 10-8 d. CuBr, Ksp = 5.0 x 10-9

The solubility of calcium carbonate (CaCO3) in water at 25 °C is 6.71 x 10-3 g/L. What is the Ksp of this sparingly soluble salt? (a) 4.5 x 10-9 (b) 1.21 x 10-12 (c) 5.47 x 10-16 (d) 8.19 x 10-3 (e) 4.06 x 10-2

The Ksp of nickel (II) hydroxide, Ni(OH)2, is 5.84 x 10-16. Calculate the solubility of this compound in g/L.

The Ksp of Ca(OH)2 is 5.5 x 10-5 at 25 °C. What is the concentration of OH- (aq) in a saturated solution of Ca(OH)2(aq)? (a) 1.9 x 10-3 M (b) 7.4 x 10-3 M (c) 2.4 x 10-2 M (d) 4.0 x 10-2 M (e) 4.8 x 10-2 M

A generic salt, AB3, has a molar mass of 351 g/mol and a solubility of 5.70 g/L at 25°C. What is the Ksp of this salt at 25 °C? AB3 (s) ⇌ A3+ (aq) + 3B- (aq)

The concentration of Pb2+ in an aqueous solution is 5.5 x 10-3 M. What concentration of SO42- is required to begin precipitating PbSO4? The Ksp of PbSO4 is 2.5 x 10-8.(a) 1.4 x 10-10 M (b) 4.5 x 10-6 M (c) 1.6 x 10-4 M (d) 8.3 x 10-4 M (e) 2.9 x 10-2 M

Ignoring activities, determine the molar solubility (S) of Zn(CN) 2 in a solution with a pH = 2.04. The Ksp for Zn(CN)2 is 3.0 times 10 -16. The Ka for HCN is 6.2 times 10 -10.

Express Ksp in terms of molar solubility, x, for a salt with a formula of

Use Ksp = 4,87 x 10-17 to calculate the solubility of iron(II) hydroxide in pure water in grams per 100.0 mL of solution.

The Ksp of PbBr2 is 6.60 x 10-6. What is the molar solubility of PbBr2 in pure water? What is the molar solubility of PbBr2 in 0.500 M KBr solution? What is the molar solubility of PbBr2 in a 0.500 M Pb(NO3)2 solution?

A generic salt, AB2, has a molar mass of 169 g/mol and a solubility of 3.60 g/L at 25°C. What is the Ksp of this salt at 25°C? AB2(s) ⇌ A2+(aq) 2B-(aq)

The molar solubility of Cu3PO4 is 3.00 x 10-4 M. Calculate the Ksp for Cu3PO4.

Question 1The solubility of a new binary salt, MX2, is 3.6 x 10-3 M. What is the value of Ksp? Question 2Calculate the solubility (in mol/L) of iron(Ill) hydroxide. Ksp = 2.8 x 10-39. Question 3Ksp for lithium carbonate is 8.2 x 10-4. What is the molar solubility of lithium carbonate?

The Ksp of cadmium carbonate, CdCO3 is 1.0 x 10-12. Calculate the solubility of this compound in g/L.

How many grams of NaOH are in 175 mL of 3.50 M NaOH? Molar masses NaOH 40.00 g/mol (a) 0.613 grams (b) 24, 500 grams (c) 50.0 grams (d) 24.5 grams (e) 613 grams

The solubility of PbCO3 is measured and found to be 9.95 x 10-5 g/L. Use this information to calculate a Ksp value for lead carbonate.

The Ksp of lead(l) hydroxide, Pb(OH)2, is 1.43 x 10-20. Calculate the molar solubility of this compound.

The Ksp of BaSO4 is 1.1 x 10-10 at 25 °C. What mass of BaSO4 (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25 °C? (a) 2.6 x 10-8 g(b) 4.5 x 10-8 g (c) 1.0 x 10-5 g (d) 1.6 x 10-4 g (e) 2.4 x 10-3 g

At a certain temperature, the solubility of strontium arsenate, Sr3(AsO4)2, is 0.0480 g. What is the Ksp of this salt at this temperature?

Two compounds with general formulas A2X and AX3 have Ksp= 1.5 x 10-5 M. Which of the two compounds has the higher molar solubility? (i) AX3 (ii) A2X

At 25°C only 0.0400 mol of the generic salt AB is soluble in 1.00 L of what is the Ksp of the salt at 25°C? AB (s) ⇌ A+ (aq) + B- (aq)

At 25°C only 0.0990 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB3 (s) ⇌ A3+ (aq) + 3B- (aq) Ksp =

What is the solubility (in mol/L) of PbCl2 given that the Ksp is 3.01 x 10-13.

At 22°C an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.14. What is the Ksp of the salt at 22°C?

Calculate the Ksp for silver sulfate if the solubility of Ag 2SO4 in pure water is 3.66 g/L Report the answer as the pKsp = - log Ksp.

At 22°C an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.28. What is the K_sp of the salt at 22°C?

The solubility product constant (Ksp) for silver (I) carbonate is 8.8 x 10-12. What is the concentration of silver ion in a saturated solution? A) 5.2 x 10-4 B) 2.1 x 10-5 C) 5.2 x 10-5 D) 1.3 x 10-4E) 2.6 x 10-4

The solubility of silver azide, AgN3(the azide ion, N3-), in water is 2.1 x 10-2 g/L. Ksp = ______

Calculate the solubility of Co(OH)2 in water at 25°C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits.

What is the value for the Ksp for a compound MX(s) if at equilibrium [M+] = 1.0 x 10-3 M? Select one: a. None of these b. 1.0 x 10-6 c. 0.0020 d. not enough information e. 1.0 x 10-3

The molar solubility of Cd3(PO4)2 is 1.19 x 10-7 mol/L at 25°C.

At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 11.05. What is the Ksp of the compound at 22 °C.

The Ksp of iron (ll) hydroxide, Fe(OH)2, is 4.87 x 10-17. Calculate the solubility of this compound in g/L.

For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g., ABC.) 1. silver sulfate A. AIPO4 2. barium sulfite B. ZnCO3 C. PbBr2 D. Pb3(PO4)2Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. silver sulfate barium sulfite

For PbBr2, Ksp = 6.60 • 10-6 M3. What is the molar solubility (S) of PbBr2? S = ___ M What is the molar solubility (S) of PbCl2 in 1.00 times 10-3 M NaCl? (For PbCl2. Ksp = 1.6 x 10-6 M3) S = ____ M

At 25°C only 0.0830 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB3 (s) ⇌ A3+ (aq) + 3B- (aq)

Calculate the solubility of Co(OH)2 in water at 25 ºC. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits.

At some specific temperature, silver bromide, AgBr(s), has a measured solubility of 6.41 x 10-7 M. Calculate the Ksp value for AgBr(s) this temperature.

Enter the solubility-product expression for Al(OH)3(s).

The Ksp of calcium hydroxide, Ca(OH)2, is 5.02 x 10-6. Calculate the molar solubility of this compound.

At 25°C only 0.0150 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB(s) ⇌ A+(aq) + B-(aq)

What is the solubility product expression for lead (II) phosphate?a. Ksp = [Pb2+]2[PO43-]3b. Ksp = [Pb2+][PO43-]c. Ksp = [Pb2+]3[PO43-]2 d. Ksp = [Pb2+][PO43-]3

What is the molar solubility of lead (II) phospate in water? (K sp = 1.0 x 10-54)a. 6.2 x 10-12 Mb. 1.4 x 10-14 Mc. 6.3 x 10-19 Md. 1.0 x 10-27 M

What is th relation between Ksp and the molar solubility, s, of lead(II) phospate?a. s2b. 4s3c. 27s4d. 108s5

The Ksp of scandium fluoride, ScF3, is 5.81 x 1024. Calculate the molar solubility of this compound.

What is the Ksp for MgF2 (s) = Mg2+ (aq) + 2 F-(aq) a. Ksp = 1/[Mg2+] [F-]b. Ksp = [Mg2+] [F-]2 c. Ksp = [Mg2+] [F-]d. Ksp = [Mg2+]2[F-]

The molar solubility of Ba3(PO4)2 is 8.89 x 10-9 M in pure water. Calculate the Ksp for Ba3(PO4)2. a. 4.94 x 10-49 M b. 5.55 x 10-41 M c. 8.16 x 10-31 M d. 6.00 x 10-39 M

The molar solubility of ZnS is 1.6 x 10-12 M in pure water. Calculate the Ksp for ZnS.a. 3.2 x 10-12 M b. 1.6 x 10-35 M c. 2.6 x 10-24 M d. 8.0 x 10-13 M

What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO 3)2? Ksp = 9.05 x 10 -18

Calculate the molar mass solubulity and the solubulity in g/L of each salt at 25°C?

C2D3 has a solubility product constant of 9.14 x 10 -9. What is the molar solubilty of C2D3?

What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO3)2? Ksp = 6.65 × 10−18 for M(OH)2.Calculate the molar solubility of lead (II) thiocyanate in 0.600 M KSCN.? K sp=2.00 x 10-5

Find the solubility in grams/L of silver chromate, Ag 2CrO4. (Ksp = 1.12 x 10-12a. 331.7b. 1.06 x 10-6c. 0.00035d. 0.022

Complete the following solubility constant expression for PbF2. Ksp = ?

Express Ksp in terms of molar solubility, x, for a salt with a formula of

When excess solid YZ is put in water and allowed to dissolve the following equilibrium reaction occurs and the equilibrium table shown can be set up.The amount of solid that dissolves is called the molar solubility, denoted here by x. Since the concentration of the solid is constant and is not included in the Ksp expression, the equilibrium expression for the reaction is Ksp=[Y][Z], or, in terms of molar solubility, Ksp = x2.Enter the the Ksp expression for the solid AB2 in terms of the molar solubility x.Express your answer in terms of x.